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IS MATTER AROUND US PURE - Coggle Diagram

- - - - Metal is a solid material which is typically hard, shiny, malleable, fusible, and ductile, with good electrical and thermal conductivity.
        
        Examples: Aluminium, Copper, Iron, Tin, Gold
      - Properties of metal
        
        Metals are malleable and ductile.
        
        Metals are good conductors of heat and electricity.
        
        Metals are lustrous (shiny) and can be polished.
        
        Metals are solids at room temperature (except mercury, which is liquid).
        
        Metals are tough and strong.
    - - Metalloids exhibit some properties of metals as well as of non-metals.
        
        Examples: Boron, silicon, germanium, arsenic, antimony, and tellurium
    - - Non-metals are brittle and are not malleable or ductile.
        They are poor conductors of heat and electricity.
        
        Examples: Carbon, Boron etc.
      - PROPERTIES OF NON [METAL)
        
        Non-metals cannot be hammered into thin sheets. ...
        
        Non-metals are not ductile. ...
        
        Non-metals are poor conductors of heat and electricity.
        
        Non-metals are not lustrous which means they are not shiny. ...
        
        Non-metals have low tensile strength. ...
        
        Non-metals are not sonorous. ...
        
        Non-metals are soft.
- - - - A mixture which has a uniform composition throughout is called a homogeneous mixture or solution.
        
        Examples: sugar in water, salt in water.
    - - A mixture which contains physically distinct parts and has a non-uniform composition is called a heterogeneous mixture.
        
        Examples: Mixture of salt and iron filings, sand and sugar.
- - - - Example: Burning of wood or paper, souring of milk.
  - - - Example: Melting of ice, boiling water.
- - - - The component of the solution that dissolves other components in it is called solvent.
    - - The component of the solution that is dissolved in the solvent is called solute.
    - - A solution is a homogeneous mixture.
      - The particles are smaller than 1 nm (10-9m) in diameter. So they are not seen with the naked eye.
      - Because of very small particle size, they do not scatter a beam of light passing through the solution. So the path of light is not visible in a solution.
      - The solute particles do not settle down when left undisturbed. That is a solution is stable.
      - The solute particles cannot be separated by the process of filtration.
    - - Solution
      - A solution is a homogenous mixture of two or more substances.
      - eg: Lemonade, soda water etc.
      - There are Solid solutions - Alloys
        
        Liquid solutions - soda water
        
        Gaseous solutions - air
      - In a solution there is homogeneity at the particle level.
        
        eg: Lemonade taste the same throughout because particles of sugar or salt are evenly distributed in the solution.
  - - - . Suspension
      - A suspension is a heterogeneous mixture in which the solute particles do not dissolve but remains suspended throughout the bulk of the medium.
      - Eg: Chalk dust and water, muddy water
    - - Properties of suspension
      - Suspension is a heterogeneous mixture.
      - The particles of the suspension can be seen with the naked eye.
      - The particles of a suspension scatter a beam of light passing through it and make its path visible.
      - The solute particles settle down when a suspension is left undisturbed. That is a suspension is unstable.
      - Particles of suspension can be separated by the process of filtration.
  - - - Colloids
      - A colloid is a heterogeneous mixture in which particles are spread uniformly throughout the solution.
      - Due to relative small size of the particles, as compared to that of suspension, the mixture appears to be homogeneous but it is a heterogeneous.
      - eg:milk, smoke etc.
      - Tyndall effect- Scattering of light by particles in a colloid or a suspension is called tyndall effect.
  - - - At any particular temperature, a solution that has dissolved as much solute as it is capable of dissolving
    - - If the amount of solute contained in a solution is less than the saturation level
    - - A solution that contains more solute than the solvent can dissolve